Which one of the following species acts as both Bronsted acid and base?

H_{2} P O_{2}^{-}

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H P O_{3}^{2 -}

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H P O_{4}^{2 -}

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All of these

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Solution

The correct option is C $H P O_{4}^{2 -}$
$H P O_{4}^{2 -} + H_{2} O ⇌ H_{2} P O_{4}^{2 -} + O H^{-}$

$H P O_{4}^{2 -} + H_{2} O ⇌ P O_{4}^{3 -} + H_{3} O^{+}$

$H_{2} P O_{2}^{-}$ is a conjugate base of $H_{3} P O_{2}$ (a monobasic acid) and does not give $H^{+}, H P O_{3}^{2 -}$ is a conjugate base of $H_{2} P O_{3}^{-}$ and does not ionise further, since $H_{3} P O_{3}$ is a dibasic acid.

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Which of the following species can act both as Bronsted acid and base?
(I) $N H_{2}^{-}$ (II) $H C O_{3}^{-}$ (III) $A l C l_{3}$ (IV)All of these

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